Write the complete, balanced chemical equation for the following reactions. Provide products where they are not given. Assume that these are all spontaneous reactions.  use soild(s), aqueous(aq), liquid(l), (g) gas in chemical equations. i. Zinc + hydrobromic acid → j. Sodium oxide + water → k. Silver carbonate + heat → l. Magnesium nitrate + ammonium phosphate → m. Hexanol (C6H11OH) + oxygen → (combustion)

Metal carbonates react with acids to form the salt of the metal and two other products, a gas and a liquid. Complete the balanced reaction of hydrochloric acid with an unknown carbonate below.

6. Eqn 1: ZnS(s) Eqn 2: S(s) + O2(g) →SO2(g) Eqn 3: ZnS(s) + O2(g)→ Zn(s) + SO>(g) → Zn(s) + S(s) AG° = +198.3 kJ AG° =-300.1 kJ The decomposition of zinc sulfide (represented by Equation 1) can be accomplished by coupling the reaction to the combustion of sulfur (represented in Equation 2), which results in the overall reaction represented in Equation 3. a. Determine the free energy change for the reaction represented in Equation 3. b. Explain why the reactions represented in Equations 1 and 2 are suitable for coupling to produce a thermodynamically favorable process.

Consider the reaction A →B with AH° = 60.55 kJ/mol,xn and the reaction B -→C with AH = 65.96 kJ/molxn- What should be the AH° in kJ/moln for the reaction A+ C→ 2 B? Report your answer to three decimal places.

A 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC.   Then the reaction is proceeded and the final temperature is reached to 28.000 oC.  Calculate the heat of reaction in kJ / mole. Hint: Treat this mixture as a diluted solution. CP of H2O(l) = 4.184 J / g oC D of H2O = 0.988 g/ mL.